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Chemistry 2000, Section A
Spring 1996 Test 1 Solutions

  1. Using the first two lines of the table, we see that the rate goes up by a factor of 5 when [A] goes up by a factor of 5. Using the last two lines, we see that the rate goes up by a factor of 4 ( tex2html_wrap_inline123 ) when the [B] goes up by a factor of 2. Therefore

    displaymath125

  2. Different amounts of reactant disappear in 0.01s so this is not a zero-order reaction. Suppose that it's a first-order reaction. Then

    displaymath127

    From the first two points, we calculate

    displaymath129

    From the next two points, we get

    displaymath131

    Since (within the accuracy of the data) we get the same rate constant in both cases, we conclude that this is a first-order reaction with tex2html_wrap_inline133 .

  3. We use the equation

    displaymath135

    The first experimental point tells us that

    displaymath137

    From the second point, we have

    displaymath139

    Subtract the two equations to eliminate tex2html_wrap_inline141 :

    displaymath143

    Therefore

    tex2html_wrap179

    Bonus:
    Substitute tex2html_wrap_inline147 into one of your two original equations and solve for tex2html_wrap_inline141 :

    displaymath151

    Use tex2html_wrap_inline153 to get the tex2html_wrap_inline155 out of the exponent. Recall that tex2html_wrap_inline155 has the same units as k:

    tex2html_wrap181

    1. The equations are obtained by applying the law of mass action:

      eqnarray51

    2. tex2html_wrap_inline163
    3. Bonus: tex2html_wrap_inline165 where tex2html_wrap_inline167 is approximately constant.
  4. If 99.9% of the plutonium has decayed, 0.1% of it remains. Put another way, we want to know how long it takes before tex2html_wrap_inline169 . We can calculate k from the half-life:

    displaymath173

    From the first-order equation, we have

    displaymath175

    which is

    tex2html_wrap183



Marc Roussel
Mon Sep 16 15:23:07 MDT 1996